At a temperature of $25^\circ C$,if $\Delta H < T \Delta S$,then $\Delta G$ = ?

The maximum work (in $kJ \, mol^{-1}$) that can be derived from the complete combustion of $1 \, mole$ of $CO$ at $298 \, K$ and $1 \, atm$ is:
[Standard enthalpy of combustion of $CO = -283.0 \, kJ \, mol^{-1}$; standard molar entropies: $S_{O_2} = 205.1 \, J \, K^{-1} \, mol^{-1}$,$S_{CO} = 197.7 \, J \, K^{-1} \, mol^{-1}$,$S_{CO_2} = 213.7 \, J \, K^{-1} \, mol^{-1}$]

For the reaction $x + y \rightarrow z$,the process is spontaneous at room temperature,and the reverse reaction is spontaneous at high temperature. Which of the following is true?

What is the work done when $1 \, \text{mole}$ of a gas expands isothermally and reversibly from $25 \, \text{L}$ to $250 \, \text{L}$ at a temperature of $300 \, \text{K}$? (in $J$)

For a spontaneous process,which of the following conditions is most favorable?

Calculate $\Delta H^{\circ}$ for a reaction at $298 \ K$ if $\Delta S^{\circ} = 120 \ J \ K^{-1}$ and $\Delta G^{\circ} = 28000 \ J$. (in $kJ$)